Answer:
[tex]C_7H_8N_4O_2[/tex]
Explanation:
Hello!
In this case, since the determination of an empirical formula is covered by first computing the moles of each atom as shown below:
[tex]n_C=\frac{46.47g}{12g/mol}=3.9mol\\\\ n_H=\frac{4.48g}{1g/mol} =4.5mol\\\\n_N=\frac{31.10g}{14g/mol} =2.2mol\\\\n_O=\frac{17.76g}{16g/mol} =1.1mol[/tex]
Now, we divide each moles by the fewest moles (those of oxygen), to obtain the subscripts in the empirical formula:
[tex]C:\frac{3.9}{1.1}=3.5 \\\\H:\frac{4.5}{1.1}=4 \\\\N:\frac{2.2}{1.1} =2\\\\O:\frac{1.1}{1.1} =1[/tex]
Thus, the empirical formula, taken to the nearest whole subscript is:
[tex]C_7H_8N_4O_2[/tex]
Whose molar mass is 180.16, therefore the empirical formula is the same to the molecular one.
Best regards!
